Chemistry Unit 9 Worksheet 1 Gases Again Answers Key

1.

The cutting edge of a pocketknife that has been sharpened has a smaller surface surface area than a boring knife. Since pressure is pressure, a sharp pocketknife will exert a higher pressure with the same amount of force and cut through textile more effectively.

iii.

Lying down distributes your weight over a larger surface expanse, exerting less pressure on the ice compared to standing upwards. If you exert less pressure, y'all are less likely to break through thin ice.

9.

Earth: 14.7 lb in^–2; Venus: i.30 × 10^three lb in⁻²

11.

(a) 101.v kPa; (b) 51 torr driblet

13.

(a) 264 torr; (b) 35,200 Pa; (c) 0.352 bar

15.

(a) 623 mm Hg; (b) 0.820 atm; (c) 83.1 kPa

17.

With a closed-stop manometer, no alter would exist observed, since the vaporized liquid would contribute equal, opposing pressures in both arms of the manometer tube. However, with an open-ended manometer, a higher force per unit area reading of the gas would exist obtained than expected, since P _gas = P _atm + P _{vol liquid}.

19.

As the bubbling rise, the pressure decreases, then their volume increases every bit suggested by Boyle's law.

21.

(a) The number of particles in the gas increases as the volume increases. (b) temperature, pressure level

23.

The curve would exist farther to the correct and college up, but the same basic shape.

33.

8.190 $\times$ 10^–2 mol; 5.553 g

35.

(a) vii.24 $\times$ 10^–2 chiliad; (b) 23.i one thousand; (c) i.five $\times$ x^–4 chiliad

41.

For a gas exhibiting ideal behavior:

43.

(a) 1.85 50 CCl₂F₂; (b) 4.66 L CH_iiiCH₂F

47.

The pressure decreases by a factor of 3.

57.

141 atm, 107,000 torr, 14,300 kPa

59.

CH_four: 276 kPa; C_twoH₆: 27 kPa; C_threeH_eight: 3.4 kPa

65.

(a) Make up one's mind the moles of HgO that decompose; using the chemical equation, make up one's mind the moles of O₂ produced by decomposition of this corporeality of HgO; and determine the volume of O₂ from the moles of O₂, temperature, and pressure level. (b) 0.308 L

67.

(a) Decide the molar mass of CCl₂F₂. From the counterbalanced equation, summate the moles of H₂ needed for the complete reaction. From the platonic gas law, catechumen moles of H₂ into book. (b) 3.72 $\times$ 10³ L

69.

(a) Balance the equation. Determine the grams of CO₂ produced and the number of moles. From the ideal gas police, determine the volume of gas. (b) 7.43 $\times$ 10⁵ L

73.

(a) 18.0 L; (b) 0.533 atm

83.

Effusion tin be divers as the process past which a gas escapes through a pinhole into a vacuum. Graham's law states that with a mixture of two gases A and B: $\left(\frac{\text{rate A}}{\text{rate B}}\right)={\left(\frac{\text{molar mass of B}}{\text{molar mass of A}}\right)}^{\mathrm{one}\text{/}\mathrm{two}}.$ Both A and B are in the same container at the same temperature, and therefore will have the aforementioned kinetic energy:
${\text{KE}}_{\text{A}}={\text{KE}}_{\text{B}}\text{KE}=\frac{1}{\mathrm{two}}\mathrm{yard}{\mathrm{five}}^2$
Therefore, $\frac{\mathrm{ane}}{2}{m}_{\text{A}}{v}_{\text{A}}^2=\frac{\mathrm{ane}}{\mathrm{two}}{m}_{\text{B}}{v}_{\text{B}}^2$
$\frac{v_{\text{A}}^2}{v_{\text{B}}^2}=\frac{k_{\text{B}}}{m_{\text{A}}}$
${\left(\frac{5_{\text{A}}^{\mathrm{two}}}{v_{\text{B}}^2}\right)}^{1\text{/}\mathrm{ii}}={\left(\frac{{\mathrm{thousand}}_{\text{B}}}{k_{\text{A}}}\right)}^{\mathrm{ane}\text{/}2}$
$\frac{v_{\text{A}}}{v_{\text{B}}}={\left(\frac{m_{\text{B}}}{{\mathrm{thousand}}_{\text{A}}}\right)}^{1\text{/}2}$

91.

Yes. At any given instant, there are a range of values of molecular speeds in a sample of gas. Any single molecule can speed up or slow down every bit it collides with other molecules. The average speed of all the molecules is abiding at constant temperature.

93.

H₂O. Cooling slows the speeds of the He atoms, causing them to behave as though they were heavier.

95.

(a) The number of collisions per unit surface area of the container wall is constant. (b) The average kinetic energy doubles. (c) The root hateful square speed increases to $\sqrt{\mathrm{two}}$ times its initial value; u _rms is proportional to $\sqrt{{\text{KE}}_{\text{avg}}}.$

97.

(a) equal; (b) less than; (c) 29.48 g mol⁻¹; (d) 1.0966 one thousand L^−one; (eastward) 0.129 k/L; (f) 4.01 $\times$ 10^v thou; internet lifting capacity = 384 lb; (k) 270 L; (h) 39.1 kJ min⁻¹

101.

The gas beliefs nearly like an ideal gas will occur nether the weather condition in (b). Molecules take loftier speeds and move through greater distances betwixt collision; they besides have shorter contact times and interactions are less likely. Deviations occur with the conditions described in (a) and (c). Under conditions of (a), some gases may liquefy. Under atmospheric condition of (c), nearly gases volition liquefy.

105.

(a) A straight horizontal line at ane.0; (b) When real gases are at low pressures and loftier temperatures, they deport close enough to platonic gases that they are approximated equally such; however, in some cases, we encounter that at a loftier pressure and temperature, the ideal gas approximation breaks down and is significantly unlike from the pressure calculated by the ideal gas equation. (c) The greater the compressibility, the more the volume matters. At low pressures, the correction factor for intermolecular attractions is more significant, and the effect of the volume of the gas molecules on Z would be a minor lowering compressibility. At higher pressures, the effect of the book of the gas molecules themselves on Z would increase compressibility (run into Figure 9.35). (d) Once over again, at low pressures, the effect of intermolecular attractions on Z would be more important than the correction factor for the volume of the gas molecules themselves, though possibly notwithstanding minor. At higher pressures and depression temperatures, the effect of intermolecular attractions would exist larger. Run into Figure 9.35. (due east) Low temperatures

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Source: https://openstax.org/books/chemistry-2e/pages/chapter-9